Method of producing lithium ion cathode materials

ABSTRACT

A method of producing Li y [Ni x Co 1−2x Mn x ]O 2  wherein 0.025≦x≦0.5 and 0.9≦y≦1.3. The method includes mixing [Ni x Co 1−2x Mn x ]OH 2  with LiOH or Li 2 CO 3  and one or both of alkali metal fluorides and boron compounds, preferably one or both of LiF and B 2 O 3 . The mixture is heated sufficiently to obtain a composition of Li y [Ni x Co 1−2x Mn x ]O 2  sufficiently dense for use in a lithium-ion battery cathode. Compositions so densified exhibit a minimum reversible volumetric energy characterized by the formula [1833−333 x ] measured in Wh/L.

CROSS-REFERENCE TO RELATED APPLICATION(S)

This application is a divisional of U.S. patent application Ser. No.10/757,645, filed Jan. 13, 2004, now allowed, which claims priority fromprovisional application 60/454,884 filed on Mar. 14, 2003, thedisclosures of which are incorporated by reference in their entiretyherein.

FIELD OF THE INVENTION

The present invention relates to lithium-ion batteries. Moreparticularly, the present invention relates to a method of densifyingcompositions useful to make electrodes for lithium-ion batteries.

BACKGROUND OF THE INVENTION

Lithium-ion batteries typically include an anode, an electrolyte, and acathode that contains lithium in the form of a lithium-transition metaloxide. Such lithium-transition metal oxides typically include LiCoO₂,LiNiO₂ and Li(NiCo)O₂. A lithium-transition metal oxide that has beenproposed as a replacement for LiCoO₂ is Li_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂which adopts the α-NaFeO₂ type structure and can be regarded as thepartial substitution of Ni²⁺ and Mn⁴⁺ (1:1) for Co³⁺ in LiCoO₂.Li_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂ materials prepared at 900° C. exhibitgood cell performance and appear to be much less reactive withelectrolytes at high temperatures compared to LiCoO₂ when charged athigh voltage. However, the material density and thus the resultingelectrode density of samples previously reported are lower than requiredfor many industrial applications of lithium-ion batteries.

Li_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂ with x being in the range of 0.25 to0.375 and y being in the range of 0.9 to 1.3 can deliver a stablecapacity of about 160 mAh/g using a specific current of 40 mA/g whencycled between 2.5 V and 4.4 V. Because both nickel and manganese areless expensive than cobalt, Li_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂ appears as apromising composition to replace LiCoO₂. One undesirable feature ofLi_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂ compounds, however, is their low densityachieved by the known synthesis of starting from a co-precipitation ofhydroxides followed by a heat treatment at about 900° C. Thisundesirable low electrode density ultimately leads to low volumetriccapacities in practical lithium-ion cells.

Denser oxides can be obtained using a synthesis constituted by a morecontrolled co-precipitation followed by treatment at temperaturesgreater than or equal to 1100° C. with a slow cooling to preserve cellperformance. Such a synthesis, however, is not completely suitable forindustrial applications because the controlled precipitation process isdifficult and is expensive due to energy requirements to achieve thehigh heat treating temperatures. Also, oxides synthesized this wayexhibit high first cycle irreversible capacity, thus limiting theiruseful capacity when used in a battery.

It is known in the art that LiF used in producingLi_(1+x)Mn_(2−x−y)M_(y)O_(4−z)F_(z) (with 0<x <=0.15, 0<y<=0.3, and0<z<=0.3, and M is a metal comprised of at least one of Mg, Al, Co, Ni,Fe, Cr), can function as a flux for lithium ion electrode materials. Theart recognizes that this compound has a spinel crystal structure.Further it is known in the art that a spinel structure requires thenominal ratio of lithium to transition-metal to oxygen in the compoundof 1:2:4. LiF is incorporated into the crystalline structure, i.e., mainphase, of the lithium transition metal oxide.

The art describes H₃BO₃ as a raw material in the synthesis ofLi[(Ni_(0.5)Mn_(0.5))_(1−x−y)M_(x)B_(y)]O₂ (where 0<=x<=0.10,0<=y<=0.05, and M is one of V, Al, Mg, Co, Ti, Fe, Cu, Zn) which can beused as a positive electrode active material. The amount of Co in thiscompound can be up to 10 atomic percent of the amount of lithium in thesynthesized lithium material. The art teaches away from increasingdensity of this material in the belief that increased density leads toinferior cell performance.

BRIEF SUMMARY OF THE INVENTION

Briefly, a method of producing Li_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂ wherein0.025≦x≦0.45 and 0.9≦y≦1.3, includes mixing [Ni_(x)Co_(1−2x)Mn_(x)](OH)₂with LiOH or Li₂CO₃ and one or both of alkali metal fluorides(preferably LiF) and boron compounds (for example, boric acid, boronoxide, and/or lithium borates), hereinafter referred to as sinteringagent, and then heating the mixture for a time sufficient to obtain adensified composition of Li_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂, the productbeing sufficiently dense for use in a lithium-ion battery. Compositionsso densified exhibit a minimum reversible volumetric energycharacterized by the formula [1833−333x] measured in Wh/L, wherein x isas previously defined, and wherein the densified compound issubstantially free of F. Preferably x has a value in the range of 0.05to 0.45 and y has a value in the range of 1.0 to 1.1.

Although dense oxides can also be obtained using a synthesis including aheating step at high temperature (1100° C.), such a heat treatment isnot considered suitable for industrial applications because 1100° C.heating places severe constraints on furnaces that do not apply forabout 900° C. heating.

In a preferred embodiment, the density is increased by using a sinteringagent involving about 0.1 to about 5.0 wt %, preferably about 0.2 toabout 3.0 wt %, more preferably about 0.5 to about 1.0 wt %, of one orboth of lithium fluoride and boron oxide at a heating temperature ofapproximately 900° C. during the synthesis ofLi[Ni_(x)Co_(1−2x)Mn_(x)]O₂.

This process provides a product with advantages of increased density,low irreversible capacity, and enhanced cathode performance such asgreater reversible volumetric energy. Useful pellet density values arein the range of about 3.3 to about 4.0 g/cm³, and preferably about 3.4to about 4.0 g/cm³.

The sintering temperature can be in the range of 800° C. to less than1100° C., preferably 850° C. to 1050° C., and more preferably about 900°C. Higher temperatures increase the processing cost and there is lessavailability of suitable processing equipment.

The lithium transition metal oxides of the invention have a layeredα-NaFeO₂ structure that requires a nominal ratio of lithium totransition metal to oxygen of 1:1:2.

BRIEF DESCRIPTION OF THE DRAWINGS

FIG. 1 shows the theoretical density (XRD) ofLi_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂ as a function of x obtained throughx-ray diffraction.

FIGS. 2 a and 2 b graphically illustrate pellet density (PD) forLi_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂ prepared at 900° C. as a function of LiFaddition for x=0.25 (FIG. 2 a) and x=0.1 (FIG. 2 b) composition.

FIG. 3 shows the BET surface area and pellet density evolutions as afunction of wt % LiF added in Li_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂ for x=0.1.

FIGS. 4 a and 4 b graphically illustrate x-ray diffraction patterns forLi_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂ for x=0.25 (FIG. 4 a) and x=0.1 (FIG. 4b) as a function of LiF addition.

FIGS. 5 a, 5 b, and 5 c graphically illustrate the effect of B₂O₃addition on the pellet density of different oxide compositions preparedat 900° C. for 3 hours for x=0.1, 0.25 and 0.375.

DETAILED DESCRIPTION OF PREFERRED EMBODIMENTS

The present invention includes a method of producing lithium transitionmetal oxides sufficiently dense for use in electrode compositions,preferably cathode compositions, for lithium-ion batteries. Compositionshaving a pellet density of greater than about 3.3 g/cm³ can be obtainedusing a sintering agent selected from the group consisting of alkalimetal fluorides (for example, LiF and/or KF; preferably LiF), boroncompounds (for example, boric acid, boron oxide, and/or lithium borates;preferably, B₂O₃), and mixtures thereof, at a level of at least about0.1 wt % of the total weight of the mixture. Higher levels of sinteringagent such as about 1.0 wt % also produce higher pellet densities. It isunderstood that when precursors have a high surface area, then greaterlevels of sintering agents can be required to produce the same increasedpellet density. Levels of sintering agent as high as about 5 wt % andeven up to about 10 wt % can produce yet even higher pellet densities.At levels of about 3 weight percent and higher, additional heating timecan be required to remove impurities from the product. Impurities of F,which would be present in a separate phase, are undesirable becausetheir presence reduces the reversible volumetric energy (RVE). Thestoichiometry of the lithium in the starting material can be adjusted tocompensate for the additional lithium being added by the use of LiF as asintering agent.

The lithium transition metal oxides of the present invention exhibitcertain characteristics that have been discovered as being useful forenhancing electrode performance. These characteristics include increaseddensity properties, without increasing the irreversible capacitysignificantly, and resulting increased electrochemical propertiesincluding RVE. A density property of interest is pellet density. Pelletdensity is that density calculated from the weight of lithium transitionmetal oxide (500 mg were used in the measurements in the examples ofthis invention) placed within a mold having a known volume (an 8 mmdiameter die was used in the measurements in the examples of thisinvention), with the lithium transition metal oxide being pressed atapproximately 48,000 psi (330,000 kPa). The resulting calculation givesa weight per volume quantity or density. The pellet density can becompared against theoretical density to ascertain the extent ofdensification of the lithium metal oxide. The theoretical density (ThD)is defined as follows:

ThD (g/ml)=[10²⁴(MW)(N)]/[(CV)(NA)],

where 1024 is the number of cubic angstroms per milliliter, MW is themolecular weight of the compound expressed in grams per mole, N is thenumber of molecular units per unit cell, CV is the volume of the unitcell expressed in cubic angstroms per unit cell and NA is Avogadro'snumber (6.023×10²³ molecular units per mole). A unit cell is a smallrepeating physical unit of a crystal structure. The type of structureand lattice constants, which together give the unit cell volume, can bedetermined by x-ray diffraction. Because the present materials have theα-NaFeO₂ structure-type, the cell volume can be calculated from thelattice constants a and c as follows:

CV=(a ²)(c)(cos(30°))

An electrochemical property of interest with regard to the presentinvention is reversible volumetric energy (RVE).

RVE=(DSC ₁)(V _(aveD))(ED)(DSC ₁ /CSC ₁).

RVE (reversible volumetric energy) (watt-hours per liter) is the amountof electrical energy stored per unit volume of the cathode electrodethat can be recycled after the first charge. RVE values of the inventionpreferably are in the range of about 1500 to about 2200 Wh/L, morepreferably in the range of about 1750 to about 2200 Wh/L.

DSC₁ (First Discharge Specific Capacity) (milliamp-hours per gram) isthe amount of electrical charge passed by a battery per gram of cathodeoxide during first discharge.

V_(aveD) (volts) is the average voltage during discharge from a battery.For the present cathode materials V_(aveD) refers to the voltage of thecathode versus lithium metal, and values of 3.85 and 3.91 V are closeapproximations Of V_(aveD) for x=0.25 and x=0.10 respectively and shallbe assumed in calculations of RVE.

CSC₁ (First Charge Specific Capacity (milliamp-hours per gram)) is theamount of electrical charge passed by a battery per gram of cathodeoxide during first charge.

ED (electrode density) (gram per milliliter) is the density of thecathode electrode, and shall be considered to be 90% of the pelletdensity.

Capacities of a battery described herein are those obtained when cyclingthe battery at 40 milliamp per gram of cathode oxide.

The lithium transition metal oxide of the present invention was preparedusing a co-precipitation process to form a transition-metal hydroxide(TMOH). The precipitated TMOH was then mixed by grinding with a combinedamount of Li(OH).H₂O and sintering agent. Li₂CO₃ can be used instead ofLiOH. After grinding, pellets were formed and then heated to about atleast 900° C. for about 3 hours, and quenched. After quenching, thepellets were ground and the resulting powder was used to make cathodes.Although pellets were made, it is understood that the ground mixture ofTMOH and lithium salts can be subjected to heat treatment withessentially the same results for a heated loose powder.

The present invention is more particularly described in the followingexamples, which are intended as illustrations only and are not to beconstrued as limiting the present invention.

EXAMPLES

The lithium metal oxides of the present invention were prepared usingthe following as starting materials: LiOH.H₂O (98%+, Aldrich ChemicalCo., Milwaukee, Wis.), CoSO₄.7H₂O (99%+, Sigma-Aldrich Co. of Highland,Ill.), NiSO₄.6H₂O (98%, Alfa Aesar, Ward Hill, Mass.), and MnSO₄.H₂O(Fisher Scientific, Hampton, N.H.). Where not designated, chemicals wereobtained from Aldrich Chemical Co., Milwaukee, Wis. All percentages wereby weight.

The process to densify lithium metal oxides of the present inventionincluded two steps. The first step involved a co-precipitation oftransition metal sulfate salts in a stirred solution of LiOH to obtain aco-precipitate. It is understood that a solution including any one ormore of LiOH, NaOH, and NH₄OH can be used as the precipitating agent,leading to the same final improvement in density described herein. Thesecond step comprised mixing the co-precipitate with stoichiometricamounts of Li(OH).H₂O and one or both of LiF and B₂O₃ (both availablefrom Aldrich Chemical Co.), forming a pellet and heating the pellet toat least about 900° C.

In performing the first step, a 100 ml aqueous solution of thetransition metal sulfates (CoSO₄.7H₂O, NiSO₄.6H₂O and MnSO₄.H₂O) (totalmetal concentration equal to 1M) was dripped into a stirred aqueoussolution of 1 M LiOH. A chemical metering pump manufactured by LiquidMetering Inc. of Acton, Mass. was used at a constant speed and strokefor 1 hour of co-precipitation. LiOH concentration was kept constantduring the co-precipitation process by metering a sufficient amount of 1M LiOH to keep the pH controlled at 14. The co-precipitant produced wasNi_(x)Co_(1−2x)Mn_(x)(OH)₂ where x is as previously defined. Theprecipitate was filtered, washed several times with distilled water,dried in air at 120° C. overnight and then ground for 5 minutes tode-agglomerate the powder.

The dried precipitate was then mixed (by grinding) with a stoichiometricamount of Li(OH).H₂O and selected amounts of one or both of LiF and B₂O₃(0, 0.2, 0.5, 1, 3, 5 wt % of the theoretical oxide mass) (AldrichChemical Co.) to keep the desired lithium stoichiometry (1 mole pertotal moles of transition metal) in the final oxide. After grinding,pellets were made, heated at 900° C., some for 3 hours and some for 6hours and then quenched between copper plates. The pellets were quenchedto save time. The pellets could have been air cooled slowly withessentially the same results. Once the pellets were cooled, they werebroken up and ground.

X-ray diffraction (XRD) was used to determine which crystalline phaseswere present in the sample and the structural characteristics of thosephases. The data was collected using an X-ray diffractometer fitted witha fixed entrance slit with 1 degree divergence, a fixed 0.2 mm receivingslit (0.06 degrees), a graphite diffracted beam monochromator, and aproportional detector for registry of the scattered radiation. A sealedcopper target X-ray source was used at generator settings of 40 kV and30 mA. Profile refinement of the collected data was made using aHill/Howard version of the Rietveld program Rietica. The structuralmodel typically used was the α-NaFeO₂ structure with Li in 3a sites, Ni,Co and Mn randomly placed on 3b sites, and oxygen atoms on 6c sites. Ananti-site defect was assumed wherein Li and Ni exchanged sites, theslight extent of which was calculated as part of the Rietveldrefinement.

Pellet density (PD) for each sintered set was obtained by making 8 mmdiameter pellets with approximately 500 mg of ground powder under apressure of 48,000 psi (30,096 kPa). The thickness and diameter of thepellet after pressing was measured and the density was then calculated.The error was estimated to be ±0.08 g/cm³.

In order to develop the correlation between pellet density and electrodedensity, test electrodes of five differentLi_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂, wherein x and y are as previouslydefined, were made. Li_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂ (90 parts), SUPER Scarbon black (5 parts) (MMM Carbon, Tertre, Belgium), and polyvinylidenedifluoride (PVDF) (5 parts) binder were combined to make electrodematerial. The electrode material was made into a slurry usingn-methylpyrrolidinone (NMP) and the slurry was then coated on aluminumfoil. The electrode material coated on aluminum foil was dried in amuffle oven overnight to evaporate the NMP and form a film. The film waspressed at 48,000 psi (330,096 kPa). Electrode density was obtained bymeasuring the thickness of the film with a digital micrometer andmeasuring the mass of a known area of the film. Five different samplesgraphically gave a slope of 0.89 when the intercept was constrained tobe zero. The achievable electrode density was thus considered to be 90%of the pellet density.

In order to perform electrochemical tests, a Bellcore-type cell wasprepared. The Bellcore-type cell included 200 to 300 mm thickPVDF/HFP-based (a copolymer of polyvinylidenefluoride/hexafluoropropylene) positive and negative electrodes and anelectrolyte separator.

The Bellcore-type cell was prepared by taking z gramsLi_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂ which was mixed with approximately 0.1(z) (by weight) SUPER S carbon black and 0.25 (z) (by weight) polymerbinder, available under the trade designation KYNAR FLEX 2801 (AtofinaChemicals, Inc. of Philadelphia, Pa.). To this mixture was added 3.1 (z)(by weight) acetone and 0.4 (z) (by weight) dibutyl phthalate (DBP),available through Aldrich Chemical Co., of Milwaukee, Wis., to dissolvethe PVDF/HFP. Several hours of stirring and shaking were required todissolve the PVDF/HFP and to break apart clumps of carbon black. Theresulting slurry was then spread on a glass plate using a notch barspreader to obtain an even thickness of approximately 0.66 mm. After theacetone had evaporated, the resulting dry film was peeled off the plateand punched into circular disks with a diameter of approximately 12 mm.The punched circular disks (electrodes) were washed several times inanhydrous diethyl ether to remove the DBP. The washed electrodes weredried at 90° C. overnight before use. The electrochemical cells wereprepared in standard 2325 (23 mm diameter, 2.5 mm thickness) coin-cellhardware with a single lithium metal foil used as both the counter andreference electrode. The cells were assembled in an argon-filledglovebox. The electrolyte used for analysis was 1M lithiumhexafluorophosphate (LiPF₆) in ethylenecarbonate-diethlycarbonate(EC/DEC) (33/67). The cells were tested using a constant charge anddischarge current of 40 mA/g (corresponding to approximately 0.6 mA/cm²)between 2.5 and 4.4V.

FIGS. 2 a and 2 b graphically illustrate the pellet density evolutionsas a function of LiF addition for Li_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂compositions for x=0.25 (FIG. 2 a) and x=0.1 (FIG. 2 b). In both cases,pellet density increased with added LiF. For x=0.1, the pellet densityincreased quasi-linearly from about 3.3 to about 3.7 g/cm³ until 1 wt %of LiF was added. The values stabilized around 3.8-3.85 g/cm³ withfurther addition of LiF. Open circles refer to special treatments. Aslight excess in lithium stoichiometry, as noted by open circle “1” inFIG. 2 b led to a slightly higher pellet density compared to theLi/M=1/1 stoichiometry where M is the total of transition metals in thecompound. Another treatment of 3 hours at 900° C. led to another slightincrease in pellet density as indicated by samples noted by open circles“2” and “3” in FIG. 2 b.

FIG. 3 shows the correlation between the decrease in BET surface areawhile the pellet density increased as a function of LiF addition in thecase of Li_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂ with x=0.1 (all samples preparedfrom the same co-precipitate). The data show the specific surface areaof Li_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂ samples prepared at about 900° C.decreased and the density increased as the weight percent of LiFincreased. Typically, electrode materials with higher specific surfacearea can lead to less-safe Li-ion cells by increasing the interface areabetween the electrolyte and the electrode grains. Lower specific surfacearea is of interest in increasing the thermal stability of the cell.

Structural data obtained from Rietveld refinements are collected inTable 1. The α-NaFeO₂ structural type was preserved in all cases andx-ray patterns and lattice constants of the starting compounds werethose typically previously observed for these compositions.

TABLE 1 Fraction of Ni Sample LiF (wt %) a (Å) c (Å) in Li-layer x = 0.10 2.8310(2) 14.135(2) 0.011(3) x = 0.1 0 2.8312(3) 14.135(2) 0.011(3) x= 0.1 0.2 2.8305(2) 14.135(2) 0.000(3) x = 0.1 0.5 2.8297(3) 14.134(2)0.013(3) x = 0.1 1 2.8294(2) 14.131(2) 0.000(3) x = 0.1 1 2.8309(2)14.132(2) 0.009(3) x = 0.1 3 2.8272(3) 14.137(2) not measured x = 0.1 3(re-heated 3 2.8282(3) 14.136(2) 0.005(3) hours) x = 0.1 5 2.8228(4)14.132(3) not measured x = 0.1 5 (re-heated 2.8234(3) 14.138(2) 0.006(3)3 hours) x = 0.1 5 (re-heated 2.8231(3) 14.142(2) 0.013(3) 6 hours) x =0.25 0 2.8493(2) 14.199(2) 0.009(3) x = 0.25 0.5 2.8508(2) 14.208(2)0.016(3) x = 0.25 1 2.8513(2) 14.210(2) 0.011(3) Parenthetical valuerefers to uncertainty in the last digit of the measurement.

The data of Table 1 show that constants a and c were unaffected by theaddition of LiF, indicating that the crystal structure dimension wasessentially free of LiF.

FIGS. 4 a and 4 b graphically illustrate similar patterns (wt % of LiFindicated on each pattern) for all samples for both compositionsLi_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂ where x=0.25 (FIG. 4 a) and where x=0.1(FIG. 4 b) regardless of whether LiF was added except with 3 and 5 wt %LiF addition for x=0.1 wherein some impurity lines clearly appeared(FIG. 4 b). For x=0.25 (FIG. 4 a), the lattice constants evolution trendwas a minimal increase as LiF increased from 0 to 1 wt % (* in FIG. 4 bindicates impurity lines).

Table 1 also lists the amount of metal defect (Ni) in the Li layer,calculated as part of the Rietveld refinement, which is known toinfluence the cell behavior. In all cases, as expected for thesecompositions, this amount was very small and no significant change wasnoticed as a function of LiF addition. Table 2 shows cycling data at 40mA/g between 2.5 and 4.4 V for Li_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O_(2.) withx=0.25 (0, 0.5 and 1 wt % LiF addition), x=0.1 (0 and 1 wt % LiFaddition) and x=0.1 (0, 0.2, 0.5, 1, 3, 3 (+3 hours) and 5 wt % LiFaddition).

Table 2 lists wt % LiF, pellet density for each sample, firstcharge/discharge energy, irreversible capacity and RVE for samples oflithium transition metal oxide where x=0.1 and 0.25.

TABLE 2 1^(st) Charge/1^(st) LiF PD Discharge % Irreversible RVE Sample(wt %) (g/cm³) (mAh/g) Capacity (Wh/L) x = 0.1 0 3.4 175/162 7.4 1794 x= 0.1 0 3.3 166/150 9.6 1574 x = 0.1 0.2 3.4 157/145 7.6 1602 x = 0.10.5 3.5 161/153 5.0 1791 x = 0.1 1 3.7 173/163 5.8 2000 x = 0.1 1 3.7157/148 5.7 1817 x = 0.1 3 3.85 141/128 9.2 1574 impurity x = 0.1 3 (re-3.94 164/149 9.1 1877 heated 3 hours) x = 0.1 5 3.8 113/96  15 1091impurity x = 0.25 0 3.2 177/165 6.8 1705 x = 0.25 0.5 3.5 173/161 6.91817 x = 0.25 1 3.6 173/155 10.4 1732 PD = Pellet Density RVE =Reversible Volumetric Energy

The data of Table 2 show that use of LiF gave improved RVE valuescompared to those when no LiF is present. Impurities in the compositionresulted in a marked decrease in RVE values. Capacity retention uponcycling maintained stable and good values with use of LiF. The cycledcapacity was the same, the RVE was improved.

Comparing Table 2 with FIG. 1, it is preferable that the lithiumtransition-metal oxides of the present invention have a pellet densityof at least about 72%, and more preferable that they have a pelletdensity of at least about 74%, of the theoretical density. Furthermore,it has been found that the reversible volumetric energy of the lithiumtransition-metal oxide of the present invention can be defined by theformula [1833−333x] as measured in Wh/L.

LiF addition had an effect on increasing the density ofLi_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂ oxides to 3.6 g/cm³ for x=0.25 and to3.7 g/cm³ for x=0.1 up to 1 wt % LiF added. This increase in density wasaccompanied by a decrease in BET surface area. Almost no influence onthe materials structure was observed. No difference at all in materialstructure was found for x=0.1 composition up to and including additionsof LiF as high as 1 wt % for lattice constants (a) and (c) (Table 1) andcell behavior (Table 2). At and above about 3 wt % addition of LiF, a“LiF impurity” containing some transition metal appeared and led tolower cell performances for the oxide. It was found that another 3 hourstreatment at about 900° C. of the 3 wt % LiF addition led to a materialwithout impurity, same lattice constants (a) and (c) as without anyadditive, and with the same cell behavior as the lower amount LiFaddition samples but having a higher density of about 3.9 g/cm³. It wasalso found that LiF additions above about 10% by weight were believed toadd fluorine to the structure of the transition metal oxide. Using otheralkali metal fluorides, such as KF as sintering agents, desirable pelletdensity values and RVE values can be obtained when using the proceduresdescribed above.

FIGS. 5 a, 5 b and 5 c graphically illustrate the effect of boron oxideaddition on the pellet density of different oxide compositions preparedat 900° C. for 3 hours. All samples for each composition were obtainedfrom the same co-precipitate. The graphs show pellet density for oxidesprepared at 900° C. for 3 hours for 3 compositions: x=0.1 (FIG. 5 a),x=0.25 (FIG. 5 b) and x=0.375 (FIG. 5 c) as a function of B₂O₃ addition.For all compositions, the pellet density increased as a function ofboron oxide content.

Table 3 lists wt % B₂O₃, pellet density for each sample, firstcharge/discharge energy, irreversible capacity and RVE for samples oflithium transition metal oxide where x=0.1 and 0.25.

TABLE 3 First Charge/First Wt % PD Discharge % Irreversible RVE SampleB₂O₃ (g/cm³) mAh/g Capacity (Wh/L) x = 0.1 0 3.3 174/154 11.5 1583 x =0.1 0.5 3.4 163/147 9.8 1586 x = 0.1 1 3.5 166/151 9.0 1692 x = 0.25 03.35 163/152 6.7 1645 x = 0.25 0.5 3.4 172/153 11.0 1603 x = 0.25 1 3.5173/147 15.0 1515

Table 3 shows that for x=0.1 the resulting increase in RVE on going from0 to 1 wt % B₂O₃ is from 1583 to 1692 Wh/L. Using other boron compounds,such as boric acid and lithium borates as sintering agents, desirablepellet density values and RVE values can be obtained when using theprocedures described above.

Although the present invention has been described with reference topreferred embodiments, workers skilled in the art will recognize thatchanges may be made in form and detail without departing from the spiritand scope of the invention.

1. A lithium transition metal oxide for use in a lithium-ion batteryhaving the general formula Li_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂, wherein0.1≦x≦0.375, and 0.9≦y≦1.3, produced by a method comprising: grinding adry precipitate of [Ni_(x)Co_(1−2x)Mn_(x)]OH₂ with a stoichiometricamount of LiOH.H₂O or Li₂CO₃ and one or both of alkali metal fluoridesand boron compounds as sintering agents to form a resulting mixture; andheating the resulting mixture until a composition ofLi_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂ having a pellet density of from about3.3 to about 3.5 g/cm³ is obtained for use in a lithium-ion battery, toform a densified composition of Li_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂ whereinthe total amount of boron compound(s) is greater than 0.2% and up toabout 10% of the total weight of the mixture, and wherein thecomposition exhibits a reversible volumetric energy of at least[1833−333x] measured in Wh/L.
 2. The lithium transition metal oxide ofclaim 1 exhibiting a pellet density of at least about 72% of theoreticaldensity.
 3. The lithium transition metal oxide of claim 1 exhibiting apellet density of at least about 74% of theoretical density.
 4. Thelithium transition metal oxide of claim 2 that is formed into a lithiumion battery electrode having a reversible volumetric energy in the rangeof 1500 to 2200 Wh/L.
 5. The lithium transition metal oxide of claim 3that is formed into a lithium ion battery electrode having a reversiblevolumetric energy in the range of 1500 to 2200 Wh/L.
 6. A lithiumtransition metal oxide for use in a lithium-ion battery having thegeneral formula of Li_(y)[Ni_(x)Co_(1−2x)Mn_(x)]O₂ wherein 0.025≦x≦0.35,and 0.9≦y≦1.3, and exhibiting a minimum reversible volumetric energycharacterized by the formula [1833−333x] measured in Wh/L.
 7. Thelithium transition metal oxide of claim 6 exhibiting a pellet density ofat least 72% of theoretical density.
 8. The lithium transition metaloxide of claim 6 exhibiting a pellet density of at least 74% oftheoretical density.
 9. The lithium transition metal oxide of claim 7that is formed into a lithium ion battery electrode having a reversiblevolumetric energy in the range of 1500 to 2200 Wh/L.
 10. The lithiumtransition metal oxide of claim 8 that is formed into a lithium ionbattery electrode having a reversible volumetric energy in the range of1500 to 2200 Wh/L.